1. III. Types of Chemical Reactions (p. 284 - 291)
Ch – Chemical Reactions
III. Types of Chemical Reactions (p )

2. Got that? SINGLE PRODUCT
A. Synthesis
Two or more substances react to produce a single product.
Got that? SINGLE PRODUCT
A + B  AB + 

3. A. Synthesis
H2(g) + Cl2(g)  2 HCl(g)

4. 2 Fe(s) + Cl2(g) → FeCl3(s) 3 2 A. Synthesis
Iron and chlorine gas react to form iron(III) chloride. 2
Fe(s) + Cl2(g) → FeCl3(s) 3 2

5. Al(s)+ Cl2(g)  2 3 2 AlCl3(s) A. Synthesis Products:
ionic – remember to cancel charges
covalent - hard to tell if names are not provided
Al(s)+ Cl2(g) 
AlCl3(s)

6. CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
B. Combustion
Oxygen combines with a substance and releases energy in the form of heat and light.
O2 is always a reactant
A + O2  B
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)

7. B. Combustion 4 2 Na2O(s) Na(s)+ O2(g)  C3H8(g)+ O2(g)  5 3 4
Products:
contain oxygen
hydrocarbons form CO2 + H2O
Na(s)+ O2(g) 
Na2O(s)
Note: this reaction is also a synthesis reaction!
C3H8(g)+ O2(g) 
CO2(g)+ H2O(g)

8. Carbon is burned in oxygen to form carbon dioxide gas.
B. Combustion
Remember: oxygen is always a reactant, and product(s) will always contain oxide.
Carbon is burned in oxygen to form carbon dioxide gas.
C(s) + O2(g) → CO2(g)

9. B. Combustion of Hydrocarbon
All hydrocarbons contain carbon and hydrogen and burn in oxygen to yield the same products – carbon dioxide and water.
CH4(g) + O2(g) → CO2(g) + H2O (g) 2 2

10. AB  A + B  + C. Decomposition Only one reactant
A single compound breaks down into 2 or more simpler substances
Only one reactant
AB  A + B  +

11. C. Decomposition
2 H2O(l)  2 H2(g) + O2(g)

12. C. Decomposition KBr(l)  2 2 K(s) + Br2(l) Products:
binary - break into elements
others - hard to tell
KBr(l) 
K(s) + Br2(l)

13. C. Decomposition
Decomposition often requires an energy source, such as heat, light, or electricity, to occur. For example, ammonium nitrate breaks down into dinitrogen monoxide and water when heated to a high temperature.
NH4+
NO3- → N2 O +
H2O
NH4NO3(s) → N2O(g) + 2H2O(g)

14. A + BC  AC + B  + + D. Single Replacement
Atoms of one element replace the atoms of another element in a compound.
metal replaces metal (+)
nonmetal replaces nonmetal (-)
A + BC  AC + B  + +

15. Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)
D. Single Replacement
Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)
Copper replaces silver

16. D. Single Replacement Balance this equation:
Potassium replaces hydrogen; therefore, potassium must be higher (more reactive) on the activity series list than hydrogen.
Balance this equation:
K(s) + H2O(l) → KOH(aq) + H2(g)

17. D. Single Replacement Fe(s)+ CuSO4(aq)  Cu(s)+ FeSO4(aq)
Products:
metal  metal (+)
nonmetal  nonmetal (-)
free element must be more active (check activity series)
Fe(s)+ CuSO4(aq) 
Cu(s)+ FeSO4(aq)
Br2(l)+ NaCl(aq) 
N.R.

18. AB + CD  AD + CB  + + E. Double Replacement
ions in two compounds “change partners”
cation of one compound combines with anion of the other
Reactions take place in aqueous solutions
AB + CD  AD + CB  + +

19. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)
E. Double Replacement
Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)

20. E. Double Replacement 2 2 Pb(NO3)2(aq)+ KI(aq)  PbI2(s)+ KNO3(aq)
Products:
switch negative ions
one product must be insoluble (check solubility table)
Pb(NO3)2(aq)+ KI(aq) 
PbI2(s)+ KNO3(aq)
NaNO3(aq)+ KI(aq) 
N.R.

21. Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)
What Type of Reactions?
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)
C(s) + O2(g) → CO2(g)
Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)

22. H2(g) + Cl2(g)  2 HCl(g)
2 H2O(l)  2 H2(g) + O2(g)